Nonmetals and Metalloids

• Life on Earth depends on certain nonmetal elements.

• The air you and other animals breathe contains several nonmetals, including oxygen.

• And all living organisms are made from compounds of the nonmetal carbon.

• Yet, while many compounds containing nonmetals are useful to life, some nonmetals by themselves are poisonous and highly reactive.

• Still other nonmetals are completely unreactive. • Compared to metals, nonmetals have a much

wider variety of properties. • However, nonmetals do have several properties

in common.

These bears, the grass behind them, and all life on Earth is based on carbon, a nonmetal.

Properties of Nonmetals

• A nonmetal is an element that lacks most of the properties of a metal.

• Most nonmetals are poor conductors of electricity and heat and are reactive with other elements.

• Solid nonmetals are dull and brittle. • Look at the periodic table. • All of the elements in green-tinted boxes

are nonmetals. • Many of the nonmetals are common

elements on Earth.

Figure 9 Periodic Table of the Elements The periodic table includes over 100 elements. Many of the properties of an element can be predicted by its position on the table.

Physical Properties

• Ten of the 16 nonmetals are gases at room temperature.

• The air you breathe is mostly a mixture of two nonmetals, nitrogen (N) and oxygen (O).

• Other nonmetal elements, such as carbon (C), iodine (I), and sulfur (S), are solids at room temperature.

• Bromine (Br) is the only nonmetal that is liquid at room temperature.

• Look at examples of nonmetals in Figure 20.

• In general, the physical properties of nonmetals are the opposite of those of the metals.

• Solid nonmetals are dull, meaning not shiny, and brittle, meaning not malleable or ductile.

• If you hit most solid nonmetals with a hammer, they break or crumble into a powder.

• Nonmetals usually have lower densities than metals.

• And nonmetals are also poor conductors of heat and electricity.

Figure 20 Physical Properties of Nonmetals Nonmetals have properties that are the opposite of metals. Comparing And Contrasting Contrast the

properties of these nonmetals with those of metals.

Chemical Properties

• Most nonmetals are reactive, so they readily form compounds.

• In fact, fluorine (F) is the most reactive element known.

• Yet, Group 18 elements hardly ever form compounds.

• Atoms of nonmetals usually gain or share electrons when they react with other atoms.

• When nonmetals and metals react, electrons move from the metal atoms to the nonmetal atoms, as shown by the formation of salt, shown in Figure 21.

• Another example is rust—a compound made of iron and oxygen (Fe2O3).

• It’s the reddish, flaky coating you might see on an old piece of steel or an iron nail.

• Many nonmetals can also form compounds with other nonmetals.

• The atoms share electrons and become bonded together into molecules.

Figure 21 Reactions of Nonmetals The table salt on a pretzel is mined from deposits found on Earth. The same compound can also be formed from a

reaction between the metal sodium and the

nonmetal chlorine.

Reading Checkpoint

• In the periodic table, most nonmetals are located – on the lower left. – on the upper right. – in the middle. – along the zigzag staircase line.

Families of Nonmetals

• Look again at the periodic table. • Notice that only Group 18 contains

elements that are all nonmetals. • In Groups 14 through 17, there is a

mix of nonmetals and other kinds of elements.

Figure 9 Periodic Table of the Elements The periodic table includes over 100 elements. Many of the properties of an element can be predicted by its position on the table.

The Carbon Family

• Each element in the carbon family has atoms that can gain, lose, or share four electrons when reacting with other elements.

• In Group 14, only carbon is a nonmetal. • What makes carbon especially important is

its role in the chemistry of life. • Compounds made of molecules containing

long chains of carbon atoms are found in all living things.

• Most of the fuels that are burned to yield energy contain carbon.

• Coal, for example, is mostly the element carbon.

• Gasoline is made from crude oil, a mixture of carbon compounds with chains of 5 to 50 or more carbon atoms in their molecules.

Figure 22 Carbon Charcoal is one form of carbon,

the only nonmetal in Group 14.

The Nitrogen Family• Group 15, the nitrogen family, contains

two nonmetals, nitrogen and phosphorus. • These nonmetals usually gain or share

three electrons when reacting with other elements.

• To introduce yourself to nitrogen, take a deep breath.

• The atmosphere is almost 80 percent nitrogen gas (N2).

• Nitrogen does not readily react with other elements, so you breathe out as much nitrogen as you breathe in.

• Nitrogen is an example of an element that occurs in nature in the form of diatomic molecules, as N2.

• A diatomic molecule consists of two atoms. • In this form, nitrogen is not very reactive. • Although living things need nitrogen, most of

them are unable to use nitrogen from the air. • However, certain kinds of bacteria can use this

nitrogen to form compounds. • This process is called nitrogen fixation. • Plants can then take up these nitrogen

compounds formed in the soil by the bacteria. • Farmers also add nitrogen compounds to the soil

in the form of fertilizers. • Like all animals, you get the nitrogen you need

from the food you eat—from plants, or from animals that ate plants.

• Phosphorus is the other nonmetal in the nitrogen family.

• Phosphorus is much more reactive than nitrogen, so phosphorus in nature is always found in compounds.

• A compound containing phosphorus is used to make matches, because it can react with oxygen in the air.

Figure 23 The Nitrogen Family

Nitrogen and phosphorus are

grouped in the same family of the periodic

table, Group 15. Making

Generalizations How do atoms of

both these elements change when they

react?

The Oxygen Family

• Group 16, the oxygen family, contains three nonmetals—oxygen, sulfur, and selenium.

• These elements usually gain or share two electrons when reacting with other elements.

• You are using oxygen right now. • With every breath, oxygen travels into your lungs. • There, it is absorbed into your bloodstream,

which distributes it all over your body. • You could not live without a steady supply of

oxygen. • Like nitrogen, the oxygen you breathe is a

diatomic molecule (O2). • In addition, oxygen sometimes forms a triatomic

(three-atom) molecule, which is called ozone (O3). • Ozone collects in a layer in the upper

atmosphere, where it screens out harmful radiation from the sun.

• However, ozone is a dangerous pollutant at ground level because it is highly reactive.

• Because oxygen is highly reactive, it can combine with almost every other element.

• It also is the most abundant element in Earth’s crust and the second-most abundant element in the atmosphere. (The first is nitrogen.)

• Sulfur is the other common nonmetal in the oxygen family.

• If you have ever smelled the odor of a rotten egg, then you are already familiar with the smell of some sulfur compounds.

• Sulfur is used in the manufacture of rubber for rubber bands and automobile tires.

• Most sulfur is used to make sulfuric acid (H2SO4), one of the most important chemicals used in industry.

Figure 24The Oxygen Family Oxygen and sulfur are the most common of the three nonmetals in

Group 16. Interpreting Tables What is the atomic number of each Group 16 element?

The Halogen Family

• Group 17 contains fluorine, chlorine, bromine, iodine, and astatine.

• These elements are also known as the halogens, which means “salt forming.”

• All but astatine are nonmetals, and all share similar properties.

• A halogen atom typically gains or shares one electron when it reacts with other elements.

• All of the halogens are very reactive, and the uncombined elements are dangerous to humans.

• Fluorine is so reactive that it reacts with almost every other known substance.

• Even water and powdered glass will burn in fluorine.

• Chlorine gas is extremely dangerous, but it is used in small amounts to kill bacteria in water supplies.

• Even though the halogen elements are dangerous, many of the compounds that halogens form are quite useful.

• Compounds of carbon and fluorine make up the nonstick coating on cookware.

• Small amounts of fluorine compounds are added to the water supply to help prevent tooth decay.

• Chlorine is one of the two elements in ordinary table salt (the other is sodium).

• Another salt of chlorine is calcium chloride, which is used to help melt snow.

• Bromine reacts with silver to form silver bromide, which is used in photographic film.

Figure 25 The Halogens The Group 17 elements are the most reactive nonmetals. Atoms of these elements easily form compounds by sharing or

gaining one electron with atoms of other elements.

The Noble Gases

• The elements in Group 18 are known as the noble gases.

• They do not ordinarily form compounds because atoms of noble gases do not usually gain, lose, or share electrons.

• As a result, the noble gases are usually unreactive.

• Even so, scientists have been able to form some compounds of the heavy noble gases (Kr, Xe) in the laboratory.

• All the noble gases exist in Earth’s atmosphere, but only in small amounts.

• Because they are so unreactive, the noble gases were not discovered until the late 1800s.

• Helium was discovered by a scientist who was studying not the atmosphere but the sun.

• Have you made use of a noble gas? • You have if you have ever purchased

a floating balloon filled with helium. • Noble gases are also used in glowing

electric lights. • These lights are commonly called

neon lights, even though they are often filled with argon, xenon, or other noble gases.

Figure 26 The Noble Gases

Electricity makes the Group 18

elements glow brightly inside glass tubes. Applying

Concepts Why are neon and the

other noble gases so

unreactive?

Hydrogen• Alone in the upper left corner of the periodic table

is hydrogen—the element with the simplest and smallest atoms.

• Each hydrogen atom has one proton and one electron.

• Some hydrogen atoms also have neutrons. • Because the chemical properties of hydrogen

differ very much from those of the other elements, it really cannot be grouped into a family.

• Although hydrogen makes up more than 90 percent of the atoms in the universe, it makes up only 1 percent of the mass of Earth’s crust, oceans, and atmosphere.

• Hydrogen is rarely found on Earth as a pure element.

• Most hydrogen is combined with oxygen in water (H2O).

Figure 27 Importance of Hydrogen Water is a compound of hydrogen and oxygen. Without liquid

water, life on Earth would be impossible.

Reading Checkpoint

• The noble gases were not discovered until the late 1800s because they are so – rare. – colorless. – light. – unreactive.

Figure 9 Periodic Table of the Elements The periodic table includes over 100 elements. Many of the properties of an element can be predicted by its position on the table.

The Metalloids

• Along the border between the metals and the nonmetals are seven elements called metalloids.

• These elements are shown in the yellow squares in the periodic table.

• The metalloids have some characteristics of both metals and nonmetals.

• All are solids at room temperature. • They are brittle, hard, and somewhat

reactive.

• The most common metalloid is silicon (Si). • Silicon combines with oxygen to form

silicon dioxide (SiO2). • Ordinary sand, which is mostly SiO2, is the

main component of glass. • A compound of boron (B) and oxygen is

added during the process of glassmaking to make heat-resistant glass.

• Compounds of boron are also used in some cleaning materials.

• The most useful property of the metalloids is their varying ability to conduct electricity.

• Whether or not a metalloid conducts electricity can depend on temperature, exposure to light, or the presence of small amounts of impurities.

• For this reason, metalloids such as silicon, germanium (Ge), and arsenic (As) are used to make semiconductors.

• Semiconductors are substances that can conduct electricity under some conditions but not under other conditions.

• Semiconductors are used to make computer chips, transistors, and lasers.

Figure 28 Silicon A silicon computer

chip is dwarfed by an ant, but the

chip’s properties as a semiconductor

make it a powerful part of modern

computers.

Reading Checkpoint

• The most common metalloid is – silicon, found in sand and glass. – boron, found in cleaning products. – germanium, found in semiconductors. – arsenic, found in transistors